Page **1** of **1**

### Number of orbitals given quantum numbers

Posted: **Tue Jul 09, 2019 10:00 pm**

by **Katherine Fitzgerald 1A**

How many orbitals can have the following quantum numbers in an atom: n=2,, l=1. m_{l}=0?

The solutions manual says the answer is 4. Can someone walk me through why / how to get there?

### Re: Number of orbitals given quantum numbers

Posted: **Tue Jul 09, 2019 10:14 pm**

by **Jeril Joseph 1B**

Not sure if this will be a helpful explanation, but I'll try. So based on the principle quantum number, we know the element being discussed in the second row of the periodic table. This means that we're dealing with the s and p orbitals. So, we know that s has one orbital and p has 3 orbitals, equaling to 4. The magnetic numbers don't apply to a specific orbital since each magnetic number can be applied to each p-orbital. Hope this helps.

### Re: Number of orbitals given quantum numbers

Posted: **Wed Jul 10, 2019 12:03 am**

by **David Zhang 1B**

Orbital number is determined by the equation n^2. With n=2, you have both l=0 (s subshell) and l=1 (p subshell). For l=0, the s subshell only has 1 orbital (0). For l=1, the p subshell has 3 orbitals (+1,0,-1). Combined, there are 4 orbitals total.

### Re: Number of orbitals given quantum numbers

Posted: **Thu Jul 11, 2019 11:40 am**

by **Yasmin Olvera 1D**

I believe it is 4 orbitals since s-shell can have 1 and p-shell can have 3.

The d-shell has 5 and f shell has 7. But since we are only going to n=2 it would be 4.